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2 years ago

Competitive inhibition occurs when a

Chemistry

2 answers:

Aleksandr-060686 [28]2 years ago

6 0

The answer to your question is C.

ioda2 years ago

3 0

Answer:

Competitive inhibition occurs when a molecule binds to an enzyme in the active site and prevents the substrate from binding. (C)

Explanation:

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Which is the most important question for deciding if a chemical reaction has occurred

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A chemical reaction undergoes a chemical change so the question you should ask if a chemical reaction has occurred is "Did a chemical change happened?". Chemical change in a reaction happens when you see bubbles, when the reaction increases or decreases in temperature or a precipitate is formed.

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3 years ago

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Which of the following is the main difference between science and pseudoscience?

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3 years ago

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3.5g of a Certain compound X, known to be made of carbon, hydrogen, and perhaps oxygen, and to have a molecular molar mass of 15

shutvik [7]

Answer:

C₅H₁₀O₅

Explanation:

1. Calculate the mass of each element in 2.78 mg of X.

(a) Mass of C

$\text{Mass of C} = \text{5.13 g CO}_{2}\times \dfrac{\text{12.01 g C}}{\text{44.01 g }\text{CO}_{2}}= \text{1.400 g C}$

(b) Mass of H

$\text{Mass of H} = \text{2.10 g H$_{2}$O}\times \dfrac{\text{2.016 g H}}{\text{18.02 g H$_{2}$O}} = \text{0.2349 g H}$

(c) Mass of O

Mass of O = 3.5 - 1.400 - 0.2349 = 1.87 g

2. Calculate the moles of each element

$\text{Moles of C = 1400 mg C}\times\dfrac{\text{1 mmol C}}{\text{12.01 mg C }} = \text{116.6 mmol C}\\\\\text{Moles of H = 234.9 mg H} \times \dfrac{\text{1 mmol H}}{\text{1.008 mg H}} = \text{233.1 mmol H}\\\\\text{Moles of O = 1870 mg O} \times \dfrac{\text{1 mmol O}}{\text{16.00 mg O}} = \text{116 mmol O}$

3. Calculate the molar ratios

Divide all moles by the smallest number of moles.

$\text{C: } \dfrac{116.6}{116.6}= 1\\\\\text{H: } \dfrac{233.1}{116.6} = 1.999\\\\\text{O: } \dfrac{116}{116.6} = 1.00$

4. Round the ratios to the nearest integer

C:H:O = 1:2:1

5. Write the empirical formula

The empirical formula is CH₂O.

6. Calculate the molecular formula.

EF Mass = (12.01 + 2.016 + 16.00) u = 30.03 u

The molecular formula is an integral multiple of the empirical formula.

MF = (EF)ₙ

$n = \dfrac{\text{MF Mass}}{\text{EF Mass }} = \dfrac{\text{150 u}}{\text{30.03 u}} = 5.00 \approx 5$

MF = (CH₂O)₅ = C₅H₁₀O₅

The molecular formula of X is C₅H₁₀O₅.

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4 years ago

Carbon atoms form ____ (2,3,4) bonds with other atoms by _____ (gaining, losing, sharing) valence electrons in order to attain a

Levart [38]

carbon atoms form 2 bonds with sharing valence electrons

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4 years ago

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The Charles Zeppelin, a fictional airship, is filled with 2.16 x 105 liters of hydrogen gas (H2). On the ground, the airship’s t

Dmitry [639]

Answer:

V2 = 3.11 x 105 liters

Explanation:

Initial Volume, V1 = 2.16 x 105 liters

Initial Temperature, T1 = 295 K

Final Temperature, T2 = 425 K

Final Volume, V2 = ?

These quantities are related by charle's law and the equation of the law is given as;

V1 / T1 = V2 / T2

V2 = T2 * V1 / T1

V2 = 425 * 2.16 x 105 / 295

V2 = 3.11 x 105 liters

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3 years ago